2 mole of an ideal at $27^{\circ} C$ expands iso - thermally and reversibly from a volume of 4 litre to 40 litre. The work done(in kJ)by the gas is:

w = -28.72 kJ

No worries! We‘ve got your back. Try BYJU‘S free classes today!

w = - 11.488 kJ

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

w = - 5.736 kJ

No worries! We‘ve got your back. Try BYJU‘S free classes today!

w = - 4.988 kJ

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B
w = - 11.488 kJ

$n = 2, T = 300 K, V_{2} = 40 l i t, V_{1} = 4 l i t, R = 8.314 / K / m o l$

Amount of work done is reversible isothermal expension

$W = - 2.303 n R T l o g (\frac{V_{2}}{V_{1}}) = - 2.303 \times 2 \times 8.314 \times 300 \times l o g (\frac{40}{4}) = - 11.488 k J$

Suggest Corrections

Similar questions

2 mole of an ideal gas at $27^{\circ} C$ expands iso - thermally and reversibly from a volume of 4 litre to 40 litre. The work done(in kJ)by the gas is:

Q. 2 mole of an ideal gas at

27^{0} C

expands isothermally and reversibly from a volume of 4 litre to 40 litre. The work done ( in kJ) by the gas is :

Q. Calculate the work done (in calorie) by 10 g of an ideal gas of molar mass 16 g in expanding reversibly and isothermally from a volume of 5 L to 15 L at 300 K.

Q. Calculate the work done by

10 g

of an ideal gas of molecular weight

44 g

in expanding reversibly and isothermaly from a volume of

5 L t o 10 L a t 300 K

Join BYJU'S Learning Program

2 mole of an ideal at 27∘C expands iso - thermally and reversibly from a volume of 4 litre to 40 litre. The work done(in kJ)by the gas is:

The correct option is B w = - 11.488 kJ n = 2,T = 300 K,V2 = 40 lit,V1 = 4 lit,R = 8.314/K/mol Amount of work done is reversible isothermal expension W = −2.303nRTlog(V2V1) = −2.303 × 2 × 8.314 × 300 × log(404) = −11.488kJ

2 mole of an ideal at $27^{\circ} C$ expands iso - thermally and reversibly from a volume of 4 litre to 40 litre. The work done(in kJ)by the gas is: